Chemical Kinetics

Question 1

How to you calculate the average rate of reaction

Answer 1

Change in Concentration/ Change in time

Question 2

For the following reaction A–>B , what is the rate of both the reactants and products?

Answer 2

Delta B / T , -1*Delta A/T .
B is produced , A is consumed

Question 3

For the following reaction 2A–>3B , what is the rate of both the reactants and products?

Answer 3

Delta B / 3T , -1* Delta A / 2T
B is produced , A is consumed

Question 4

What is the formula for the instantaneous rate of reaction?

Answer 4

Rate = d[reactant]/ time = d[product]/time

Question 5

What is the Rate Law for the reaction A+B –> C

Answer 5

Question 6

For the reaction A–> B
Rate = k[A]^n
We double the concentration of A
What is the observed change in Rate for
n= 0
n=1
n=2

Answer 6

=0 No change
= 1 Double
=2 Quadrouple

Question 7

What is the purpose of an integrated rate law

Answer 7

allow us to predict the rate at any time in the progress of reaction

Question 8

Derive the integrated rate law for the following reaction
A–> B
rate = k[A]^0

Answer 8

Question 9

Derive the integrated rate law for the following reaction
A–> B
rate = k[A]^1

Answer 9

Question 10

Derive the integrated rate law for the following reaction
A–> B
rate = k[A]^2

Answer 10

Question 11

Draw a graphical plot for the following reaction
A–> B
rate = k[A]^0

Answer 11

Question 12

Draw a graphical plot for the following reaction
A–> B
rate = k[A]^1

Answer 12

Question 13

Draw a graphical plot for the following reaction
A–> B
rate = k[A]^2

Answer 13

Question 14

what is a half life

Answer 14

amount of time for half of the reactant to disappear

Question 15

As Temperature increases, why does this have a big impact on the rate of reaction?

Answer 15

Molecular movement increases (Kinetic Energy increases)

Number of particles above the activation energy increase

Both increase the number of successful collisions per second

10 Degreee increase = double rate of reaction

Question 16

What is the Energy of Activation

Answer 16

Energy required to break the bonds , to form an Activated complex

Question 17

Label the Energy of Activation and Enthalpy of Reaction on this Reaction Profile

Answer 17

Question 18

What is the Arrhenius equation?

Answer 18

Question 19

Explain how a catalyst increases the rate of reaction.

Answer 19

Lowers the activation energy.
By forming Activated states with the reactants,
aiding them to react together.

Doesnt get used up.

Question 20

Determine the rate law and Rate Perimeter for the following reaction

Answer 20

Question 21

The Rate Parameter is highly dependent on Temperature in the Arrhenius equation, the rate ___________________________ increase in temperature

Answer 21

The Rate Parameter is highly dependent on Temperature in the Arrhenius equation, the rate doubles with a 10 degree increase in temperature